If K_eq is ____ compared to 1 an equilibrium mixture of reactants and products will contain very little of the reactants compared to the products

very large

If K_eq is very large compared to 1 an equilibrium mixture of reactants and products will contain

very little of the reactants compared to the products

If K_eq is ____ compared to 1 an equilibrium mixture of reactants and products will contain very little of the products compared to the reactants

very small

If K_eq is very large compared to 1 an equilibrium mixture of reactants and products will contain

very little of the products compared to the reactants

If K_eq is ____ compared to 1 an equilibrium mixture of reactants and products will contain approximately equal amount of reactants and products

close to 1

If K_eq is close to 1 compared to 1 an equilibrium mixture of reactants and products will contain

approximately equal amount of reactants and products

In an exothermic reaction adding heat will cause the reaction to

shift to the left

In an endothermic reaction adding heat will cause the reaction to

continue forward faster

An adiabatic process occurs when

no heat exchange occurs in a system

An isothermal process occurs when

temperature of the system remains constant

Isobaric process occurs when

pressure of the system remains constant

An isolated system occurs when

it cannot exchange energy or matter with its surroundings

A closed system occurs when

it can exchange energy but not matter with its surroundings

An open system occurs when

it can exchange energy and matter with its surroundings

To find the heat moved in a given process

q = m*c*dT

m=mass
c=specific heat
dT=change in temp

Given:
Several reactions and their changes in enthalpy. Calculate change in enthalpy for another reaction based on this.

Comine given reactions, multiply/factor to cancel needed compounds on either side after adding is complete so that the final reaction is the same as the one that must be calculated for. Add the reactions' dH's to find the dH for the answer.

Change in entropy is given by

dS=Sfinal-Sinitial
dS=q_rev/T

Change in Gibbs free energy is found by

dG = dH - TdS

If dG is negative the reaction is _______

spontaneous

If dG is positive the reaction is _______

not spontaneous

If dG is zero the reaction is ______

in a state of equilibrium

If dH = TdS the reaction is ____

in a state of equilibrium

If dH > TdS the reaction is ____

not spontaneous

If dH < TdS the reaction is ____

spontaneous

If dG is ____ the reaction is spontaneous

negative

If dG is ____ the reaction is not spontaneous

positive

If dG is _____ the reaction is in equilibrium

zero

The heat of formation of any element in its elemental state is

0

P1V1=?

P2V2

V1/T1=?

V2/T2

n1/V1=?

n2/V2

PV=?

nRT

P1V1
____ = ?
T1

P2V2
____
T2

density = ?

m/v

P(MM)
_____
RT

KE=(1/2)mv^2=

(3/2)kT

KE=

(1/2)mv^2
(3/2)kT

r1/r2 = ?

sqrt(MM2/MM1)

Natural processes want to decrease ____ and increase ____

enthalpy
entropy

Natural processes want to ____ enthalpy and _____ entropy

decrease
increase

Any process that increases entropy and decreases enthalpy will be

spontaneous at any temperature

Any process that does this will be spontaneous at any temperature

increase entropy
decrease enthalpy

The higher the molecular mass, the ___ the gas will diffuse

slower

The ____ the molecular mass, the slower the gas will diffuse.

higher

To find bond order from a MO diagram:

subtract antibonding(*) electrons from bonding electrons and divide by two